Ionic Bonding. Recall some information…. The number of valence electrons = group number for an element. Elements in the same group have similar chemical properties. Valence electrons are largely responsible for giving an element its chemical properties.
Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.
Lewis Dot Structures can show us how many valence electrons an element contains. Notice, all Group 1A elements have one valence electron.
When atoms form compounds they achieve the electron configuration of a noble gas.
The bonds of friendship are hard to break
Befriends Sad Halogen
Formed when an atom gains or loses electrons; the atom will take on a charge (+ or -).
Sodium has one electron in its outermost shell
1. Gain 7 electrons
2. Lose 1 electron
Sodium now has a complete outer shell; but now has one fewer electron than before!
Sodium is now an ion and has a +1 charge.
Magnesium now has two more protons than electrons, giving it a positive charge.
Aluminum is in group 3; therefore it needs to lose 3 valence electrons.
Aluminum now has three more protons than electrons, giving it a positive charge.
Fluorine has 7 electrons in its outermost shell
1. Gain 1 electron
2. Lose 7 electron
Fluorine is now an ion and has a -1 charge.
Fluorine now has a complete outer shell; but now has one more electron than before!
-2 both of them.
Oxygen now has 2 more electrons than protons, giving it a negative charge.
Oxygen has 6 valence electrons; it needs to gain 2.
Nitrogen has 5 valence electrons; it needs to gain 3.
Nitrogen now has 3 more electrons than protons, giving it a negative charge.
Review your Ions POGIL packet for more information!
All Group both of them.7A elements are gaining 1 electron (remember to get to 8); they will ALL have a -1 charge.
All Group 6A elements are gaining 2 electrons; they will ALL have a -2 charge.
All Group 1A elements are losing their only valence electron; they will ALL have a +1 charge.
All Group 2A elements are losing both of their valence electrons; they will ALL have a +2 charge.
Ionic Compounds both of them.
Compounds composed of cations and anions; electrically neutral (even though ions have charges); properties of the compounds can be very different from the properties of the ions.
This group 1A element needs to lose 1 electron; it transfers it to the group 7A element, which needs to gain 1 electron.
Both atoms are now happy with full octets!
Note: This slide uses Lewis Dot Structures
This both of them.cation has a +2 charge. The anions have -1 charges. This means you need two anions to bond with the cation.
1(2) + 2(-1) = 0
This cation has a +2 charge. The anion has a -2 charge. This you only need one of each to form the ionic bond.
1(2) + 1(-2) = 0
#cation(charge) + #anion(charge) = 0
Review the PHET (Sugar and Salt Solutions) simulation for more information!
For more examples, head over to the videos section on mrgarcia.netand watch the Ionic Bonding examples.
This is what I would expect you to do on an exam, I must see the arrows for you to receive credit!